Magnesium And Oxygen Conjoin In A Whole-Number Ratio

2. Obtained a 2-3 cm strip of magnesium metal ribbon and coiled it loosely into a small ball. Added the magnesium metal to the acid in the test tube.

) Suppose that some magnesium oxide smoke had escaped during the investigation, the Mg:O ratio would have increased from 58% to 72%. The final mass of MgO would have decreased because the magnesium oxide smoke is part of the product and when some of it escapes, it decreases the final mass.

III. For observation 1 and 2, pour 1 cup of water into a pan and place on stove on high heat. For observation 2 add

Hypothesis/Prediction: The percent composition by mass of magnesium in magnesium oxide will not change significantly with each group that conducted the experiment. The composition of each substance should stay the same and any differences must be due to some error.

Trial 2: Mass of fired crucible, lid, and hydrated salt (g) – Mass of fired crucible and lid (g) = Mass of hydrated salt (g) = 48.057g - 47.760g = 0.297g

They heated it for another 10 minutes, that time adding a little bit of distance between the flame and crucible bottom. They allowed the crucible to cool for about 10 minutes. Then they reweighed the sample for 6 more minutes, cooled it and then weighed it again.

Based on my and other classmates' observations and results it can be proved that every time magnesium combines with oxygen to form Magnesium oxide the percent composition for magnesium will be 60.31% and for oxygen it will be 30.69 % (the results achieved by experiments are

Weigh the large block on an electronic balance and write the mass on the data table. Record the masses of the metal blocks in grams and maintain the certainty of either the milligram or analytical balance. When you are finished recording show your data to your instructor for their initials.

red powder, heating it, weighing it, reheating it, and weighing it again until we reached a constant mass, we were able to determine the

10) Calculate the mass of oxygen that was added to the magnesium. (see hint in data table)

In this lab, we will create a chemical reaction between the reactants oxygen (O2) and magnesium (Mg) using combustion. The product will be magnesium oxide (MgO). In this lab we will record the masses of reactants and products to perform stoichiometry of the chemical equation Mg + O2 -> MgO. The actual yield of product will differ from the theoretical yield based on how the experiment is performed. The independent variable is the product amounts and the dependent variable is the percent yield.

The objective of this lab was to find the empirical formula of magnesium oxide. In order to produce magnesium oxide. In this experiment, magnesium reacted in an oxygen-rich environment while inside of a crucible. The masses before and after the oxidation were both measured. The masses that were resulted were then used to calculate the empirical formula of magnesium oxide. The simplest whole-number in the form of a ratio in which atoms join and form a compound is known as the empirical formula. By finding the percent composition of each element in the compound you are able to determine the empirical formula. When finding the empirical formula it is important to know how to find things such as the limiting reagent, percent yield along with the theoretical yield. The limiting reagent is a substance that will not let the reaction proceed because of its presence. The percent yield and the theoretical yield are both found by comparing the reaction and the experimental yield and recording those results.

After that, measure and record the mass of the crucible under the “After Heating” section of the

The purpose of this experiment is to determine the mass of a piece of the magnesium, without weighing the magnesium on a balance. To determine the mass of the magnesium, without weighing is to use stoichiometry of a chemical reaction to be able to determine the mass of the magnesium. If the volume of hydrogen gas produced can be determined by using the combined gas law equation, then the mass of magnesium being used can be determined using

Low temp for drying the sample , then the wall is heated up to 1400 K for short period to ash the sample, then up to 2550 K for few seconds to produce gas phase atoms.